Kc for Methyl Methanoate??

Hey! I'm just in the process of doing my Salters Chemistry Investigation.

Does anyone know what the equilibrium constant for the hydrolysis of Methyl Methanote is?

Reply 1

parag

Well the equation I think is:

HCOOCH3(aq) + H2O(l) <-> HCOOH(aq) + CH3OH(aq)

So Kc = [HCOOH][CH3OH]/[HCOOCH3]

The value depends on the concentrations of each, so without those I don't think you can work it out

Reply 2

MatHor

The Kc is constant for all concentrations provided the temperature remains constant. I have managed to find it for ethyl ethanoate, just can't find it for methyl methanoate! :frown:

Reply 3

dfghj

I'm pretty sure you need the initial concentration of methyl methanoate to work out the =m constant. Unless you just mean an expression for Kc for this reaction, which would be:

[CH3OH][HCOOH / [CH3COOH][H20]

Unless you have the Kc for the esterification (in which case the Kc value of the hydrolysis would be 1/Kc of esterification), I don't know.

Reply 4

vinny221

youll have to look it up in a data book or else calculate it from the values youve been given

Reply 5

Tommy07

is methyl methanoate the same thing as ethanoate??

Reply 6

vinny221

no, methyl mentanoate is HCOOCH3 whilst methyl ethanoate is CH3COOCH3. The ethanoate comes from the carboxylic acid, ethanoic acid. methanoate is derived from methanoic acid.

Reply 7

Tommy07

my bad! i was getting confused between esters and ketones! thanx vinny.

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